Find Kc for the reaction 2 NO(g) + O2(g) ↔ 2NO2(g),  given Kp = 2.2 x 1012 @ 25 °C.  R = 0.08206 L.atm/mol.K

Carbon monoxide reacts with water according to the following equilibrium reaction: CO (g) H2O (g) CO2 (g) + H2 (g) For this reaction, K = 0.810 at a temperature of 1000.°C. Calculate the value of AG for this reaction at 1000.ºC. %3D

12. Consider the chemical reaction 2HCl(g) H2(g) + Cl2(g). It contains 8.0 mol HCI, 0.20 mol H₂ and 0.40 mol Cl₂ in a 1.00 L flask at equilibrium. Calculate Kc and Kp at 300. °C. for the reaction.

You are given the following:   H2 (g) + Br2 (g) 2 HBr (g) Kp = 7.9 x 1011                            H2 (g) 2 H (g) Kp = 4.8 x 10-41                                         Br2 (g) 2 Br (g) Kp = 2.2 x 10-15 What is Kp for the reaction shown below?                                H (g) +  Br (g)   HBr (g) Kp = ?

3. Phosphoryl chloride, POCI3(g), is used in the manufacturing of flame retardants. It is manufactured in an equilibrium process in which phosphorus trichloride reacts with nitrogen dioxide to form POCI3(8)and NO(g) according to the following equation: PCI3 (g) + NO2 (g) = POCI3 (g) + NO (g) The Keg for this reaction at 800 K is 6.90. If 1.25 mol PCI3 (g) and 1.94 mol NO2 (g) are placed into a 2.0 L container, what is the concentration of each gas at equilibrium at 800 K? PCI3 (g) NO2 (g) POCI3 (g) NO(g) Keq = 6.90 + + E

The reaction mixture below contains 0.305 atm of H2, 0.060 atm of S2, and 0.420 atm of H2S. 2 H2S(g) 2 2 H2(g) + S2(g) Kp = 2.4x104 at a particular temperature. Based on the information provided, select the correct relationship. K; the reaction will proceed to form more S2(g). Q > K; the reaction will proceed to the left. O More experimental data are needed to answer a question of this type. Q = K; the reaction is at equilibrium and no change is expected.

Nitrogen dioxide reacts to form dinitrogen tetroxide as follows: 2 NO2 N₂04 (g) At 150 °C, Kp = 4.51. If one starts with 10.0 atm NO2 (g), what is the equilibrium pressure (in atm) of N₂O4 (g)?

For the following reaction: NH4Cl(s) ↔ NH3(g) + HCl(g) ΔH = +42.1 kilocalories Suppose the substances in the reaction above are at equilibrium at 600K in volume V and at pressure P. State whether the partial pressure of NH3(g) will have increased, decreased, or remained the same when equilibrium is reestablished after each of the following disturbances of the original system. Some solid NH4Cl remains in the flask at all times. Justify each answer with a one-or-two sentence explanation. (e) A quantity of gaseous NH3 is added. The answer for e states that the partial pressure of NH3 is increase, which is a bit confusing. The explanation is that some of the the added NH3 reacts with HCl to relieve stress but only part of NH3 reacts. Can you explain how and where this is implied in the reaction or question. Would appreciate a lot of clarification

Consider the following equilibrium: 2NH3(g) → N₂(g) + 3H₂(g) AG = 34. kJ Now suppose a reaction vessel is filled with 6.39 atm of ammonia (NH3) and 0.200 atm of hydrogen (H₂) at 206. °C. Answer the following questions about this system: Under these conditions, will the pressure of NH3 tend to rise or fall? Is it possible to reverse this tendency by adding N₂? In other words, if you said the pressure of NH3 will tend to rise, can that be changed to a tendency to fall by adding N₂? Similarly, if you said the pressure of NH3 will tend to fall, can that be changed to a tendency to rise by adding N₂? If you said the tendency can be reversed in the second question, calculate the minimum pressure of N₂ needed to reverse it. Round your answer to 2 significant digits. OO U rise fall yes no atm x10 X Ś

If Kc = 0.0095 for the reaction below at 298.0 K, then what is the value of Kp? (R = 0.0821 L.atm/mol.K.) 3 A (g) + B (g) C (g) + D (g) 1 4 7 +/- 2 LO 5 8 3 6 9 0 X C x 100 +